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- (12) V. Consider the titration of a 25.0-mL sample of 0.175 M CH3NH2 (Kb = 4.40 x 104) with 0.150 M HBr. What is the pH of the solution after 10.0 mL of the acid have been added? What is the pH at the equivalence point?A student determined the concertration of NaOCI in a commercial bleach sample using the same technique described in section "F" of the Halogens and Their Compounds lab. The student required 18 drops of 0.01M Na25203 to reach the end point. What is the concentration (reported in percentage) of NaOCI in the bleach sample?A 50.0 mL solution of Ca(OH)2 with an unknown concentration was titrated with 0.340 M HNO3. To reach the endpoint, a total of 26.2 mL of HNO3 was required. Write the balanced chemical equation for the reaction 3c2₂²- 1 + 2 (s) H 3 Ca ( Reset 4 (1) N LO 5 6 7 (g) OH 8 NO₂ 9 (aq) NO3 0
- A 1.000- g sample of a sweetening agent containing soluble saccharin was treated with 20.00 mL of 0.0500M AgNO3. The reaction is: Saccharin-Na + Ag+ → Saccharin-Ag (s) + Na+ After removal of the solid, titration of the filtrate and washings required 2.51mL of 0.0610M KSCN. Calculate percent of saccharin in the sample.As a technician in a large pharmaceutical research firm, you need to produce 250. mLmL of 1.00 MM potassium phosphate buffer solution of pHpHpH = 6.85. The pKapKa of H2PO4−H2PO4− is 7.21. You have the following supplies: 2.00 LL of 1.00 M KH2PO4M KH2PO4 stock solution, 1.50 LL of 1.00 M K2HPO4M K2HPO4 stock solution, and a carboy of pure distilled H2OH2O. How much 1.00 M KH2PO4M KH2PO4 will you need to make this solution?7:36 .l LTE 7 Unanswered •1 attempt left • Due on Oct 6, 7:00 PM 5.0 mL of 3.6 M K2CO3 solution is diluted to make a 0.45 M solution, what is the volume of the diluted solution? А 5.0 mL 10. mL C 20. mL D 40. mL 80. mL Submit B
- A certain local brand of “healthy” chicharon was found to contain 0.4132 g of NaCl after Fajan titration. How much sodium is present in the sample? MM NaCl=58.44 g/mol; MW Na+= 22.99 g/mol; MW Cl =35.45 g/mol 0.1626 mg 105.4 mg 0.1054 mg 162.6 mg5 The amount of ascorbic acid, C6HSO6, in orange juice was determined by oxidizing the ascorbic acid to dehydroascorbic acid, C6H6O6, with a known excess of I3, and back titrating the excess Is with Na2S2O3. A 5.00-mL sample of filtered orange juice was treated with 50.00 mL of excess 0.01023 M I3. After the oxidation was complete, 13.82 mL of 0.07203 M NazS2O3 was needed to reach the starch indicator end point. Report the concentration of ascorbic acid in milligrams per 100 mL.The tetraethyl lead Pb(C2H5)4 in a 25.00 mL sample of aviation gasoline was shaken with 15.00 mL of 0.02179 M I2. (Hint: one mole of I2 reacts with one mole of the tetraethyl lead). After the reaction was complete, the unused I2 was titrated with 7.37 mL of 0.02959 M thiosulfate solution. Calculate the weight of Pb(C2H5)4 (MW = 323.4 g/mol) in each liter of gasoline.
- Q3/ A 0.80868 gm sample of a commercial phosphate detergent was ignited at a red heat to destroy the organic matter the residue was then taken up in hot HCl, which converted the P to H3PO4. The phosphate was precipitated as MgNH₂PO4.6H₂O by addition of Mg¹2 followed by aqueous NH3 after being filtered and washed. The precipitate was converted to Mg₂P₂O(222.57gm mol) by ignition at 1000 C this residue weighed represent 61.5% of the total sample mass. Calculate the percent P(30.974gm mol),O (16 gm/mol) and Mg (24.3 gm/mol) in the sample.In the preparation of the standard curve for protein analysis, 50 mn BSA (bovine serum albumin) dissolved in H2O to a final volume of 5 mL was used as stock solution. What is the weight of BSA in 0.1 mL of stock solution? In 0.2 mL?What is the Qsp of a solution mixture Al(OH)3 formed from 10 mL 1.00M C6H5NH2 and 15 mL 0.10M Al(NO3)3?